`Delta_(r) G^(@)= - RT " In K. For the same reaction at the same temperature using " K_(c) and K_(p) " the values "Delta _(r)G^(@) " ` are found to be different . Why ?

Explanation

To understand why the values of ΔrG° (standard Gibbs free energy change) are found to be different when calculated using Kc (equilibrium constant in terms of concentration) and Kp (equilibrium constant in terms of partial pressure) for the same reaction at the same temperature, we can break down the explanation into several steps.

### Step-by-Step Solution:

1. **Understanding ΔrG° and its Relation to K**:
The equation ΔrG° = -RT ln K relates the standard Gibbs free energy change (ΔrG°) to the equilibrium constant (K) of a reaction at a given temperature (T). Here, R is the universal gas constant and T is the temperature in Kelvin.

2. **Differentiating Between Kc and Kp**:
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